Consider the reaction: CO(g)+2 H2(g) ⟶CH3 OH(g) A reaction...

Consider the reaction: $$ \mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{OH}(g) $$ A reaction flask initially contains 112 torr of $\mathrm{CO}$ and 282 torr of $\mathrm{H}_{2}$. The reaction is allowed to proceed until the pressure stops changing, at which point the total pressure is 196 torr. Determine the percent yield for the reaction. Assume a constant temperature and that no other reactions occur other than the one indicated.

Consider the reaction:
$$
\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{OH}(g)
$$
A reaction flask initially contains 112 torr of $\mathrm{CO}$ and 282 torr of $\mathrm{H}_{2}$. The reaction is allowed to proceed until the pressure stops changing, at which point the total pressure is 196 torr. Determine the percent yield for the reaction. Assume a constant temperature and that no other reactions occur other than the one indicated.

Key Concepts

Reaction Stoichiometry

Reaction stoichiometry involves interpreting the balanced chemical equation to determine the proportions in which reactants combine and products form. This concept is key to calculating how much of each reactant is consumed and the resulting amount of product based on the mole ratios given by the reaction coefficients.

Limiting Reagent Determination

Identifying the limiting reagent is crucial for predicting the maximum amount of product that can be formed in a reaction. This concept entails comparing the available amounts of reactants (or, in the case of gases, their partial pressures) relative to the stoichiometric requirements of the reaction to ascertain which reactant will be completely consumed first.

Utilization of Partial Pressures in Gas Reactions

In reactions involving gases under constant temperature and volume, partial pressures serve as a direct measure of the molar amounts. This concept leverages the ideal gas law, allowing the use of pressure measurements to infer mole ratios, which is especially useful in assessing reaction progress and changes in the system.

Percent Yield Calculation

The percent yield is a quantification of how efficiently a reaction produces the desired product and is determined by comparing the actual yield to the theoretical yield predicted by stoichiometry. This concept is particularly important in real-world applications, where the actual yield is often less than the computed maximum yield due to various practical limitations.

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